Question 1

Calculate the pH of a 0.800 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Accepted Answer

A)  2.70
B)  4.40
C)  9.60
D)  11.30E) B) and C)
F) All of the above

Question 2

Which one of the following can behave either as a Br∅nsted-Lowry acid or a Br∅nsted-Lowry base in an aqueous solution reaction?

Accepted Answer

A)  HSO4-
B)  CH4
C)  HI
D)  H3PO4E) A) and B)
F) A) and C)

Question 3

An Arrhenius acid is best defined as a

Accepted Answer

A)  electron pair donor.
B)  proton acceptor.
C)  substance that dissociates in water to produce aqueous hydrogen ions.
D)  substance that dissociates in water to produce aqueous hydroxide ions.E) None of the above
F) A) and B)

Question 4

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A)  LiHSO4
B)  NaClO4
C)  KF
D)  CH3NH3IE) A) and C)
F) A) and B)

Question 5

A proton hydrated by ten water molecules has the formula ________.

Accepted Answer

The answer of A proton hydrated by ten water molecules...

Question 6

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion.

Accepted Answer

A)  4.00 × 10-9 M
B)  4.00 × 10-10 M
C)  4.00 × 10-11 M
D)  5.00 × 10-11 ME) C) and D)
F) B) and C)

Question 7

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A)  KHSO4
B)  RbClO4
C)  BaO
D)  CH3CH3NH3BrE) None of the above
F) A) and B)

Question 8

Ammonia NH3,has a base dissociation constant of 1.8 × 10-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

Accepted Answer

A)  NH4+,1.9 × 109
B)  NH4+,1.8 × 10-5
C)  NH4+,5.6 × 10-10
D)  NH2-,5.6 × 10-10E) B) and C)
F) None of the above

Question 9

The Br∅nsted-Lowry acids in the chemical equation below are ________ and ________.
HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq)

Accepted Answer

Question 10

What is the hydronium ion concentration of a 0.300 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq) .

Accepted Answer

A)  2.3 × 10-2 M
B)  4.2 × 10-2 M
C)  2.3 × 10-3 M
D)  4.2 × 10-3 ME) None of the above
F) All of the above

Question 11

A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A)  acidic,3.08 × 10-9 M
B)  acidic,3.08 × 10-10 M
C)  basic,3.08 × 10-9 M
D)  basic,3.08 × 10-10 ME) B) and D)
F) B) and C)

Question 12

Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water.

Accepted Answer

A)  HSO4-(aq) + H2O(l) ⇌ H2SO4(aq) + OH-(aq) 
B)  HSO4-(aq) + H2O(l) ⇌ SO42-(aq) + H3O+(aq) 
C)  HSO4-(aq) + H2O(l) ⇌ SO32-(aq) + OH-(aq) 
D)  HSO4-(aq) + H2O(l) ⇌ SO3(g) + OH-(aq) + H2O(l) E) A) and B)
F) A) and C)

Question 13

Phenobarbital has a pKa = 7.4.Compared to a 1.0 × 10-3 M solution,1.0 × 10-4 M phenobarbital will have a ________ (higher,lower)pH and a ________ (higher,lower)percent ionization.

Accepted Answer

Question 14

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A)  NaI
B)  KBr
C)  RbCl
D)  CsFE) All of the above
F) A) and B)

Question 15

What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH) 2 with enough water to produce a total volume of 250.00 mL?

Accepted Answer

A)  2.10
B)  2.40
C)  11.60
D)  11.90E) B) and D)
F) A) and C)

Question 16

When dissolved in water,which of the following compounds is an Arrhenius acid?

Accepted Answer

A)  HCN
B)  NaOH
C)  NaF
D)  CH3CH2OHE) A) and B)
F) All of the above

Question 17

What is the conjugate base of the Br∅nsted-Lowry acid HPO42-?

Accepted Answer

A)  H3PO4
B)  H2PO4-
C)  HPO42-
D)  PO43-E) All of the above
F) C) and D)

Question 18

In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq) + H2O(l) ⇌ H3O+(aq) + CN-(aq)

Accepted Answer

A)  HCN
B)  H2O
C)  H3O+
D)  CN-E) A) and D)
F) C) and D)

Question 19

What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?

Accepted Answer

A)  hydrofluoric acid with Ka = 3.5 × 10-4
B)  benzoic acid with Ka = 6.5 × 10-5
C)  acetic acid with Ka = 1.8 × 10-5
D)  hypochlorous acid with Ka = 3.5 × 10-8E) B) and C)
F) A) and B)

Question 20

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H2O) 63+(aq) + 6 CN-(aq) → Fe(CN) 63-(aq) + 6 H2O(l)

Accepted Answer

A)  Fe3+
B)  H2O
C)  CN-
D)  Fe(H2O) 63+E) A) and B)
F) All of the above

Exam 15: Aqueous Equilibria: Acids and Bases

What is the conjugate base of the Br∅nsted-Lowry acid HPO42-?

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In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq) + H2O(l) ⇌ H3O+(aq) + CN-(aq)

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Phenobarbital has a pKa = 7.4.Compared to a 1.0 × 10-3 M solution,1.0 × 10-4 M phenobarbital will have a ________ (higher,lower)pH and a ________ (higher,lower)percent ionization.

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When dissolved in water,which of the following compounds is an Arrhenius acid?

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What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH) 2 with enough water to produce a total volume of 250.00 mL?

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Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

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What is the hydronium ion concentration of a 0.300 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) ⇌ H3O+(aq) + CH3CO2-(aq) .

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Ammonia NH3,has a base dissociation constant of 1.8 × 10-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

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What is the strongest monoprotic acid of the following set if all the acids are at 0.100 M concentration?

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Which one of the following can behave either as a Br∅nsted-Lowry acid or a Br∅nsted-Lowry base in an aqueous solution reaction?

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Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

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Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion.

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An Arrhenius acid is best defined as a

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Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

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Calculate the pH of a 0.800 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

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Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H2O) 63+(aq) + 6 CN-(aq) → Fe(CN) 63-(aq) + 6 H2O(l)

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A proton hydrated by ten water molecules has the formula ________.

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A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

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The Br∅nsted-Lowry acids in the chemical equation below are ________ and ________. HNO2(aq)+ H2O(l)⇌ H3O+(aq)+ NO2-(aq)

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Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO4- in water.

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What is the conjugate base of the Br∅nsted-Lowry acid HPO₄^2-?

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In the following chemical equation indicate the reactant that is a Br∅nsted-Lowry base. HCN(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CN^-(aq)

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Phenobarbital has a pK_a = 7.4.Compared to a 1.0 × 10^-3 M solution,1.0 × 10^-4 M phenobarbital will have a (higher,lower)pH and a (higher,lower)percent ionization.

Correct Answer
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Correct Answer
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What is the pH of a solution prepared by diluting 50.00 mL of 0.020 M Ba(OH) ₂ with enough water to produce a total volume of 250.00 mL?

Correct Answer
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Correct Answer
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What is the hydronium ion concentration of a 0.300 M acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq) + H₂O(l) ⇌ H₃O⁺(aq) + CH₃CO₂^-(aq) .

Correct Answer
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Ammonia NH₃,has a base dissociation constant of 1.8 × 10^-5.What is the conjugate acid of ammonia and what is its acid dissociation constant?

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Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-4 M in hydroxide ion.

Correct Answer
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Correct Answer
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Calculate the pH of a 0.800 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-9.

Correct Answer
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Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H₂O) ₆³⁺(aq) + 6 CN^-(aq) → Fe(CN) ₆^3-(aq) + 6 H₂O(l)

Correct Answer
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Correct Answer
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A solution with a hydrogen ion concentration of 3.25 × 10^-5 M is and has a hydroxide ion concentration of .

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The Br∅nsted-Lowry acids in the chemical equation below are and . HNO₂(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ NO₂^-(aq)

Correct Answer
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Write a balanced equation for the dissociation of the Br∅nsted-Lowry acid HSO₄^- in water.

Correct Answer
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